Explanation

• The forward reaction is exothermic because ΔH = −94 kJ/mol, meaning heat is released during the formation of SO₃.
• Increasing temperature shifts the equilibrium towards SO₂ and O₂, reducing the equilibrium constant Kp.
• According to Le Chatelier’s principle, increasing pressure shifts the equilibrium towards SO₃ because the product side has fewer moles of gas (2 moles) than the reactant side (3 moles).
• A catalyst speeds up both forward and reverse reactions equally.
• It does not change the equilibrium constant or the equilibrium yield of SO₃.

Last verified on 25-10-2026

Explanation

• Metals above hydrogen in the electrochemical series generally have more negative standard reduction potentials and tend to lose electrons more readily than hydrogen.
• Hydrogen acts as the cathode when it gains electrons and undergoes reduction in a galvanic cell where such a metal acts as the anode.
• The metal above hydrogen acts as the anode and as the reducing agent because it loses electrons and reduces another substance.

Last verified on 25-10-2026

Explanation

• Electrochemistry is the branch of chemistry that studies the relationship between electrical energy and chemical energy, including their interconversion.
• It deals with electrochemical cells, batteries, electrolysis, and oxidation-reduction (redox) reactions.
• Galvanic cells convert chemical energy into electrical energy.
• Electrolytic cells use electrical energy to drive chemical reactions.

Last verified on 25-10-2026

Explanation

• Elastic potential energy is stored when a spring is stretched or compressed.
• This energy is released when the spring returns to its original shape.

Additional information:

• Kinetic energy is the energy of motion.
• Chemical energy is stored in chemical substances.

Last verified on 23-10-2026

Explanation

• An electron carries a negative electric charge.
• Its charge is approximately −1.602 × 10⁻¹⁹ C.
• A proton has an equal magnitude of positive charge, while a neutron has zero electric charge.
• The charge of an electron is called the elementary charge with a negative sign.

Explanation

Oxidation is the chemical process of:

• Losing electrons
• Oxidation state increases
• Always paired with reduction (together form redox)
• Reducing agent gets oxidized (it gives up the electrons)

Additional information 

Reduction:

• Gain electrons
• Oxidation state lowers
• Always paired with oxidation (redox)
• Oxidizing agent gets reduced

Last verified on 22-10-2026

Explanation

• Arsenic is a toxic substance that can contaminate groundwater and cause serious health problems after prolonged exposure.
• Water sources confirmed to have excessive arsenic should be clearly marked, and people should be advised not to use them for drinking or cooking.

Last verified on 21-10-2026

Explanation

• Nitrogen (N₂) makes up about 78% of Earth's atmosphere. 
• It is generally not considered an air pollutant in its normal form.

Additional information:

• Hydrocarbons can contribute to air pollution by reacting with nitrogen oxides to form ground-level ozone.
• Chromium, especially certain compounds such as hexavalent chromium, can pollute the air and pose serious health risks.
• Carbon dioxide (CO₂) is a greenhouse gas that contributes to global warming and is also classified as an air pollutant in some environmental frameworks.

Last verified on 21-10-2026

Explanation

• Sulphur dioxide (SO₂) is used as a dechlorinating agent to remove residual chlorine from water.
• It reacts with chlorine and reduces it to chloride ions, thereby neutralizing its disinfecting effect.
• Dechlorination is commonly required when excess chlorine must be removed from treated water or wastewater.

Last verified on 17-10-2026

Explanation

• Amino acids are the building blocks of proteins.
• Proteins are formed when amino acids join together by peptide bonds.
• Proteins are essential for growth, repair, and body functions.
• There are 20 standard amino acids used to make proteins.

Verified & Updated